Solutions & Solubility Quiz

What is the driving force behind the movement of solute molecules through the stagnant layer in the process of dissolution?

• Viscosity of the solvent

• Pressure exerted by the solute molecules

• Temperature difference between the solute and solvent

• Difference in concentration between the solute at the surface and the farthest side of the stagnant layer

Which factor can enhance the solution rate of a solute?

• Increasing the thickness of the stagnant layer

• Decreasing the saturation solubility

• Decreasing the particle size

• Increasing the pH of the solution

What is the effect of temperature on the solubility of sodium sulfate?

• Solubility increases with temperature up to a certain point, then decreases

• Solubility decreases with temperature

• Solubility is not affected by temperature

• Solubility remains constant with temperature

How does the molecular structure of a compound affect its solubility?

• Changes in molecular structure can have a marked effect on solubility

• Molecular structure has no impact on solubility

• Decreasing molecular weight increases solubility

• Increasing molecular weight decreases solubility

What is the common ion effect in the context of solubility?

• The solubility of a salt is inversely proportional to the common ion concentration

• The solubility of a salt is not affected by the presence of another salt

• The solubility of one salt is increased by the presence of another having a common ion

• The solubility of one salt is reduced by the presence of another having a common ion

How does the addition of a solubilizing agent affect the solubility of a substance?

• Forms large aggregates in solution to increase solubility

• Decreases solubility by forming complexes with the solute

• Has no effect on solubility

• Reduces the surface area of the solute to decrease solubility

What is the effect of pH on the solubility of weak acids?

• Weak acids are less soluble in both acidic and alkaline solutions

• Weak acids are more water-soluble in an alkaline solution

• Weak acids are more water-soluble in an acidic solution

• Weak acids have constant solubility regardless of pH

How does the formation of a complex affect the solubility of a substance?

• Has no effect on solubility

• Increases solubility by decreasing the surface area of the solute

• Decreases solubility by reducing interactions with the solvent

• Increases solubility by forming intermolecular complexes

What is the solubility product Ksp used for in the context of slightly soluble electrolytes?

• Describes the solubility of a compound in a saturated solution

• Determines the color of a compound in solution

• Indicates the pH at which a compound is most soluble

• Measures the rate of dissolution of a compound

How does the presence of an added substance affect the solubility of slightly soluble electrolytes?

• Increases solubility by decreasing the temperature of the solution

• Has no effect on solubility

• Increases solubility by forming complexes with the solute

• Reduces solubility by competing for the aqueous solvent